Question

When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction...

When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction

CaCO3(s)→CaO(s)+CO2(g)

What is the mass of calcium carbonate needed to produce 77.0 L of carbon dioxide at 1 bar and 273 K?

Express your answer with the appropriate units.

Homework Answers

Answer #1

Given:

P = 1.0 bar

= (1.0/1.01325) atm

= 0.9869 atm

V = 77.0 L

T = 273.0 K

find number of moles using:

P * V = n*R*T

0.9869 atm * 77 L = n * 0.08206 atm.L/mol.K * 273 K

n = 3.391 mol

This is mol of CO2 formed

From balanced equation,

moles of CaCO3 required = moles of CO2 formed

= 3.391 mol

Molar mass of CaCO3,

MM = 1*MM(Ca) + 1*MM(C) + 3*MM(O)

= 1*40.08 + 1*12.01 + 3*16.0

= 100.09 g/mol

mass of CaCO3,

m = number of mol * molar mass

= 3.391 mol * 100.09 g/mol

= 339 g

Answer: 339 g

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